AngryPancake

Maybe it’s not automated and whoever is responsible isn’t awake yet.

Your user is still linked to your home instance. If that goes down, you don’t have access to it. You can still browse Lemmy from other servers.

Honestly, the small scale racism is a huge issue. These constant small arguments is what manifests it in people’s heads.

But yeah Trump is an ass, fuck him.

Or right click the back button

I’ll write an explanation here, but I’ll try to answer all questions from the thread. Also quantum mechanics is complicated, so sorry for the long text.

Electron orbitals are weird and complicated, for hydrogen we can solve them analytically and depending on the quantum number of the energy levels we are looking at, they take the forms as in the picture on Wikipedia:

https://upload.wikimedia.org/wikipedia/commons/thumb/e/e7/Hydrogen_Density_Plots.png/1280px-Hydrogen_Density_Plots.png

Now whatever energy levels and quantum numbers are, what we are seeing is the probability of the location of the outer most electron (ok hydrogen only has one).

To understand bonds, we don’t really need the picture of orbitals, but what’s important is understanding that electrons occupy shells. A certain number of atoms can fit into a shell and when it’s full, the electrons start a new shell. It gets complicated quickly with more electrons, however in the simpler case, a shell can fit 2n^2 electrons, where n is the shell number. So for n=1, a maximum of 2 electrons can fit, for n=2, a maximum of 8 electrons can fit.

Shells want to be filled, so that leads to two possible bond types. If an atom with a free electron comes close to an atom that has a free spot for an electron, the electron can hop over to the other atom, at which point we have an ionic bond (the atom that loses the electron loses one electric charge and is thus positively charged, the other atoms gains an electric charge and is then negatively charged, so they want to be together).

Another option is covalent bonding, where instead of an electron jumping to another atom, the atoms actually share the electron.

Now do orbitals overlap? I wouldn’t give that question a yes or no, because, at that level, we can’t really separate atoms anymore. When the atoms are far apart we can draw separate orbitals for both, but when they get together, new orbitals form that is the solution of the electronic configuration of the new molecule we just created. It’s more like the orbitals that we have get deformed into new orbitals.

I’d like to tinker with the hardware but unfortunately it’s just not necessary. Love the device

Same for me. I started practicing it a while ago, but whenever I woke up I felt like I didn’t sleep at all

It’s a shame that all of the bee’s food reserves are sold

I wanted to see for myself and it looks like the spectra of the sun and moon are fairly similar:

Moon: https://olino.org/blog/us/articles/2015/10/05/spectrum-of-moon-light/comment-page-1/

Sun: https://seos-project.eu/earthspectra/images/Solar-spectrum_th.png

Looks pretty similar I gotta say

That being said, the intensity is of course much lower of the light reflected from the moon.

Why would you want to have two homes in the same city? It’s hard enough finding one apartment, if people go around having multiple accommodations, it’s just unfair for everyone else.